1. Acids, Bases, and Salts

2. Writing Names for Acids
2 types of acids - binary and ternary (sometimes called oxy)
binary - H and one other type of atom
name them hydro ic acid
Ex1 HCl
Ex2 HBr
Ex3 HF
Ex4 H2S
Ex5 H3P

3. Writing Formulas for Acids
Writing formulas from names for Acids - use the “criss-cross applesauce” rules.
Ex6 Hydronitric Acid
H3N

4. Writing Names for Acids
Ternary (oxy) Acids
acids that have H with a polyatomic ion
Do not start with Hydro-
Change the –ate ending to –ic (I ate something icky
Change the – ite ending to –ous (The bug bite was poisonous)

5. Writing Names for Acids
Ex7 H2SO4
Sulfuric Acid 
Ex8 H2SO3 
Sulfurous Acid  
Ex9 HClO4
Perchloric Acid
Ex10 HClO3  
Chloric Acid 
Ex11 HClO2  
Chlorous Acid

6. Writing Formulas for Acids
When writing formulas from names, use the “criss-cross applesauce” rules.
Ex12 Nitric Acid
HNO3
Ex13 Phosphorous Acid
H3PO3

7. Writing Names for Salts & Bases
Salts and bases are really just ionic compounds (we named these in Ch 9)
Binary ionic compounds - composed of only two types of elements. Ending of nonmetal changes to – ide.
Ex1: NaCl Ex2 MgCl2
Ex3 : Al2O3 Ex4 NaH
- Binary ionic transition metals – 1 element can have more than 1 charge
Ex 5:
CuCl Cu = +1 Copper I Chloride
CuCl2 Cu = +2 Copper II Chloride
Do sauce apple cross criss to figure out the charge and write it in the name as a Roman Numeral

8. Writing Names for Salts & Bases
Ternary Ionic Compounds - 3 or more elements make up the compound
polyatomic ions are present. OH- is a polyatomic ion and it also classifies a substance as a base.
Ex6 LiClO3 
Ex7 LiClO2 
Ex8 CaCO3   
Ex9 Na(OH)

9. Writing Formulas for Bases & Salts
Look up the charges for the ions on the P-table
Criss Cross Applesauce
if the charges are the same, “drop ‘em”
if the charges are different, “criss cross”
charges the same -
Ex1 Sodium Chloride
Na+1 Cl-1  NaCl
Ex2 Magnesium Sulfide
Mg+2 S-2  MgS
charges different -
Ex3 Sodium Sulfide
Na+1 S-2  Na2S
Ex4 Magnesium Chloride
Mg+2 Cl-1  MgCl2

10. Writing Formulas for Bases & Salts
Polyatomic ions – Still criss cross charges
if you take a polyatomic ion, more than once, use parentheses......
Ex5 Sodium Nitrate
Na+1 NO3-1  NaNO3 
Ex6 Magnesium Hydroxide
Mg+2 OH-1  Mg(OH)2

11. 19.1 Acid-Base Theories Properties of Acids 1. Sour Taste
Ex: Citrus Fruits like lemons, limes, and oranges
2. Aqueous solutions of acids are electrolytes because they ionize in water.
Aqueous Solution – A solution that has water as the solvent
Electrolyte – Solute that when dissolved in solution will conduct electricity.
Ionization - Molecules undergo a chemical change and turn into ions through the dissolving process.
HCl(g) + H2O  H+ (aq) + Cl-(aq) *more on this later
H2SO4(g) + H2O  2H+(aq) + SO42- (aq)

12. Properties of Acids: 3. Causes indicators to change colors
Indicator – a dye that appears one color in an acid and a different color in a base.
4. Reacts with metals to form H2 gas and salt.
Mg HCl (aq)  MgCl 2(aq) + H 2(g)
5. Reacts with bases to form salt and water
This is called neutralization.
It’s really just a double replacement reaction.
HCl(aq) + NaOH(aq) NaCl(aq) + HOH (l)
3H2SO4(aq)+ 2Al(OH)3(aq)  Al2(SO4)3(aq) HOH (aq)

13. Some common acids:
Sulfuric – used for fertilizer, petroleum, production of metal, paper, paint
HCl – stomach acid, food processing, iron, steel
Acetic acid – vinegar, fungicide, produced by fermentation
Nitric acid – explosives, rubber, plastics, dyes, drugs
Phosphoric acid – beverage flavoring, animal feed, detergents

14. 19.1 Acid-Base Theories Properties of Bases 1. Bitter Taste
Ex: Baking Chocolate
2. Aqueous solutions of bases are electrolytes because they dissolve by dissociation.
Dissociation- The separation of ions that occurs when an ionic compound dissolves
NaOH(s) H2O  Na+(aq) + OH-(aq)
Mg(OH)2(s) H2O  Mg+2(aq) + 2OH-(aq)

15. 19.1 Acid-Base Theories Properties of Bases
3. Causes indicators to change colors
4. Slippery Feel
Ex: Soap
5. Reacts with acids to form salt and water (neutralization)
HCl(aq) + NaOH(aq) NaCl(aq) + HOH (l)

16. Arrhenius Acids and Bases
1887, Swedish chemist Svante Arrhenius define acids and bases in a new way.
Arrhenius Acid – A Hydrogen-containing compound that separates in aqueous solution to yield hydrogen ions (H+)
HCl(g) + H2O  H+ (aq) + Cl-(aq)
We now know H+ are not found alone when in solution. Instead, the ions join to water molecules to form hydronium ions (H3O+)
Hydronium ion – the ion that forms when a water molecule gains a hydrogen ion.

17. Arrhenius Acids and Bases
Arrhenius Base- A compound that when dissolved in water forms hydroxide ions (OH-)
NaOH(s) +H2O Na+(aq) + OH- (aq)
KOH(s) + H2O  K+(aq) + OH-(aq)

18. Reactions of Acids and Bases
1. Neutralization (same as double replacement reactions learned earlier in the year):
Acid Base  Salt Water
HX MOH  MX H2O
Ex1:
HCl(aq) + NaOH(aq)  NaCl(aq) + HOH(l)

19. Reactions of Acids and Bases
2. Acid + Metal (single replacement reactions learned earlier in the year):
Metal + Acid  Salt + Hydrogen
Ex2:
Mg(s) HCl(aq)  MgCl2(aq) H2(g)

20. Reactions of Acids and Bases
3. Ionization of an acid (Acid in water):
Acid + Water  Hydronium Ion + Negative Ion
Ex3:
HCl(g) + H2O(l)  H3O+1(aq) + Cl-1(aq)

21. Reactions of Acids and Bases
4. Dissociation of Bases (base that ends with OH in water):
Base + Water  Positive Ion Hydroxide
Ex4:
Fe(OH)3(s) + H2O(l)  Fe+3(aq) + 3 OH-1(aq)

22. A closer look at Neutralization Reactions
Remember – Neutralization reactions are when an acid and a base react to form salt and water. They can also be written as….
Net Ionic Equations - typically used for double replacement reactions and other reactions taking place in aqueous solutions

23. Net Ionic Equations
write an equation & show ALL soluble compounds as dissociated ions
write a net ionic equation – only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution and does not include
spectator ions - ions found on the reactants and products side

24. Net Ionic Equations Molecular
HBr(aq) + Li(OH)(aq) ---> LiBr(aq) + H(OH)(l)
Total ionic
H+(aq)+Br-(aq)+Li+(aq)+(OH)-(aq) ---> Li+ + Br-(aq)+ H(OH)(l)
NET IONIC
“spectator ions” are crossed off
H+(aq) (OH)-(aq) ---> H2O(l) (net ionic equation)

25. Net Ionic Equations HCl+ Na(OH) Molecular Total Ionic Net Ionic
Spectator Ions